Ch.1 - Intro to General ChemistryWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Classification of Matter
Physical & Chemical Changes
Chemical Properties
Physical Properties
Intensive vs. Extensive Properties
Scientific Notation
SI Units
Metric Prefixes
Significant Figures
Significant Figures: Precision in Measurements
Significant Figures: In Calculations
Conversion Factors
Dimensional Analysis
Density of Geometric Objects
Density of Non-Geometric Objects
Additional Practice
The Scientific Method
Standard Deviation, Mean, Median & Mode
Accuracy & Precision

Significant Figures are used to determine some level of accuracy within our recorded measurements. 

The Rules for Significant Figures

Concept #1: Significant Figures

Example #1: Determine the number of significant figures in the following value: 0.003840

Practice: How many sig figs does each number contain?

a) 100. min                                                          

b) 17.3 x 103 mL

c) 10 apples

Practice: Indicate the number of significant figures in the following: 

A liter is equivalent to 1.059 qt. 

Practice: How many significant figures are contained in the following measurement? 

3,482,005 mg